Question

gibbs free energy of the reaction (kj/mol) reaction progress reaction is endergonic and it favors the product formation reaction is exergonic and it favors the reactant formation reaction is endergonic and it favors the reactant formation reaction is exergonic and it favors the product formation

Explanation:

Exergonic reactions have a negative change in Gibbs - free energy ($\Delta G<0$), meaning the products have lower free - energy than the reactants. In the given graph, the free - energy of the products ($P$) is lower than that of the reactants ($R$), so $\Delta G<0$ and it is an exergonic reaction. Exergonic reactions are spontaneous and favor the formation of products.

Answer:

Reaction is Exergonic and it favors the product formation